CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313203
Among \({\rm{O,}}{{\rm{O}}^{\rm{ + }}}{\rm{,}}{{\rm{O}}^{{\rm{2 + }}}}\,\,{\rm{and}}\,\,{{\rm{O}}^{{\rm{2 - }}}}\), the species having most negative value of \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\) are respectively.
Successive electron affinity always decrease \({\text{O}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{\text{ - }}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( - \right){\rm{ve}}\) \({{\text{O}}^{{\text{ - }}}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{{\text{2}}\,{\text{ - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{ + }}} \right){\rm{ve}}\) \({\text{O}}\xrightarrow{{{\text{ + 2e}}}}{{\text{O}}^{{\text{2 - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{Total}}} \right){\rm{ = ( + )ve}}\) Thus, \({{\rm{O}}^{{\rm{2 - }}}}\) will show most positive \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\), while \({{\rm{O}}^{{\rm{2 + }}}}\) will show most negative value due to small size.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313204
Assertion : Noble gases have large positive electron gain enthalpy. Reason : Electron has to enter the next higher principal quantum level.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Noble gases exhibit large positive electron gain enthalpies (EGE) because the addition of an electron requires it to enter the next higher principal quantum level, resulting in a highly unstable electronic configuration. So option (1) is correct
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313205
Which of the following configuration will have least electron affinity?
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313206
Assertion : Electron affinity of oxygen is more negative than nitrogen but less negative than fluorine. Reason : N, O, F belong to same period of the periodic table.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Nitrogen has an highly stable half filled configuration of \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{3}\) and addition of an electron to it is not easy. But oxygen has a greater tendency to add electron as its p orbital is incomplete \(\left(1 s^{2}, 2 s^{2}, 2 p^{4}\right)\). Easier the addition of an electron to the atom, more negative the electron gain enthalpy. N, O, F belong to \(2^{\text {nd }}\) period of the periodic table. but there is no relation between these two statements. So, option (2) is correct.
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CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313203
Among \({\rm{O,}}{{\rm{O}}^{\rm{ + }}}{\rm{,}}{{\rm{O}}^{{\rm{2 + }}}}\,\,{\rm{and}}\,\,{{\rm{O}}^{{\rm{2 - }}}}\), the species having most negative value of \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\) are respectively.
Successive electron affinity always decrease \({\text{O}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{\text{ - }}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( - \right){\rm{ve}}\) \({{\text{O}}^{{\text{ - }}}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{{\text{2}}\,{\text{ - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{ + }}} \right){\rm{ve}}\) \({\text{O}}\xrightarrow{{{\text{ + 2e}}}}{{\text{O}}^{{\text{2 - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{Total}}} \right){\rm{ = ( + )ve}}\) Thus, \({{\rm{O}}^{{\rm{2 - }}}}\) will show most positive \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\), while \({{\rm{O}}^{{\rm{2 + }}}}\) will show most negative value due to small size.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313204
Assertion : Noble gases have large positive electron gain enthalpy. Reason : Electron has to enter the next higher principal quantum level.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Noble gases exhibit large positive electron gain enthalpies (EGE) because the addition of an electron requires it to enter the next higher principal quantum level, resulting in a highly unstable electronic configuration. So option (1) is correct
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313205
Which of the following configuration will have least electron affinity?
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313206
Assertion : Electron affinity of oxygen is more negative than nitrogen but less negative than fluorine. Reason : N, O, F belong to same period of the periodic table.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Nitrogen has an highly stable half filled configuration of \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{3}\) and addition of an electron to it is not easy. But oxygen has a greater tendency to add electron as its p orbital is incomplete \(\left(1 s^{2}, 2 s^{2}, 2 p^{4}\right)\). Easier the addition of an electron to the atom, more negative the electron gain enthalpy. N, O, F belong to \(2^{\text {nd }}\) period of the periodic table. but there is no relation between these two statements. So, option (2) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313203
Among \({\rm{O,}}{{\rm{O}}^{\rm{ + }}}{\rm{,}}{{\rm{O}}^{{\rm{2 + }}}}\,\,{\rm{and}}\,\,{{\rm{O}}^{{\rm{2 - }}}}\), the species having most negative value of \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\) are respectively.
Successive electron affinity always decrease \({\text{O}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{\text{ - }}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( - \right){\rm{ve}}\) \({{\text{O}}^{{\text{ - }}}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{{\text{2}}\,{\text{ - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{ + }}} \right){\rm{ve}}\) \({\text{O}}\xrightarrow{{{\text{ + 2e}}}}{{\text{O}}^{{\text{2 - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{Total}}} \right){\rm{ = ( + )ve}}\) Thus, \({{\rm{O}}^{{\rm{2 - }}}}\) will show most positive \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\), while \({{\rm{O}}^{{\rm{2 + }}}}\) will show most negative value due to small size.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313204
Assertion : Noble gases have large positive electron gain enthalpy. Reason : Electron has to enter the next higher principal quantum level.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Noble gases exhibit large positive electron gain enthalpies (EGE) because the addition of an electron requires it to enter the next higher principal quantum level, resulting in a highly unstable electronic configuration. So option (1) is correct
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313205
Which of the following configuration will have least electron affinity?
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313206
Assertion : Electron affinity of oxygen is more negative than nitrogen but less negative than fluorine. Reason : N, O, F belong to same period of the periodic table.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Nitrogen has an highly stable half filled configuration of \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{3}\) and addition of an electron to it is not easy. But oxygen has a greater tendency to add electron as its p orbital is incomplete \(\left(1 s^{2}, 2 s^{2}, 2 p^{4}\right)\). Easier the addition of an electron to the atom, more negative the electron gain enthalpy. N, O, F belong to \(2^{\text {nd }}\) period of the periodic table. but there is no relation between these two statements. So, option (2) is correct.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313203
Among \({\rm{O,}}{{\rm{O}}^{\rm{ + }}}{\rm{,}}{{\rm{O}}^{{\rm{2 + }}}}\,\,{\rm{and}}\,\,{{\rm{O}}^{{\rm{2 - }}}}\), the species having most negative value of \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\) are respectively.
Successive electron affinity always decrease \({\text{O}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{\text{ - }}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( - \right){\rm{ve}}\) \({{\text{O}}^{{\text{ - }}}}\xrightarrow{{{\text{ + e}}}}{{\text{O}}^{{\text{2}}\,{\text{ - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{ + }}} \right){\rm{ve}}\) \({\text{O}}\xrightarrow{{{\text{ + 2e}}}}{{\text{O}}^{{\text{2 - }}}}\) \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}{\rm{ = }}\left( {{\rm{Total}}} \right){\rm{ = ( + )ve}}\) Thus, \({{\rm{O}}^{{\rm{2 - }}}}\) will show most positive \({\rm{\Delta }}{{\rm{H}}_{{\rm{eg}}}}\), while \({{\rm{O}}^{{\rm{2 + }}}}\) will show most negative value due to small size.
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313204
Assertion : Noble gases have large positive electron gain enthalpy. Reason : Electron has to enter the next higher principal quantum level.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Noble gases exhibit large positive electron gain enthalpies (EGE) because the addition of an electron requires it to enter the next higher principal quantum level, resulting in a highly unstable electronic configuration. So option (1) is correct
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313205
Which of the following configuration will have least electron affinity?
CHXI03:CLASSIFICATION OF ELEMENTS AND PERIODICITY IN PROPERTIES
313206
Assertion : Electron affinity of oxygen is more negative than nitrogen but less negative than fluorine. Reason : N, O, F belong to same period of the periodic table.
1 Both Assertion and Reason are correct and Reason is the correct explanation of the Assertion.
2 Both Assertion and Reason are correct but Reason is not the correct explanation of the Assertion.
3 Assertion is correct but Reason is incorrect.
4 Assertion is incorrect but Reason is correct.
Explanation:
Nitrogen has an highly stable half filled configuration of \(1 \mathrm{~s}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{3}\) and addition of an electron to it is not easy. But oxygen has a greater tendency to add electron as its p orbital is incomplete \(\left(1 s^{2}, 2 s^{2}, 2 p^{4}\right)\). Easier the addition of an electron to the atom, more negative the electron gain enthalpy. N, O, F belong to \(2^{\text {nd }}\) period of the periodic table. but there is no relation between these two statements. So, option (2) is correct.